Unit 3

Question 1

Kinetic Molecular Theory (KMT) Definitions:

Answer 1

-Ignore the Volume
-Motion Causes Pressure
-Particles do not affect each other
-Average KE is proportional to temperature in Kelvin\

Question 2

P and V ( T= Constant)

Answer 2

Inversamente Proporcional

Question 3

P and T (V = constant)

Answer 3

Directamente Proporcional

Question 4

V and T (P = Constant)

Answer 4

Directamente Proporcional

Question 5

V and n (P and T = Proportional)

Answer 5

Directamente Proporcional

Question 6

Daltons Law

Answer 6

P is independent of the type of gas molecule

Question 7

KMT Particle Masses

Answer 7

Have same KE at given temperature

Question 8

KE Formula

Answer 8

KE = 1/2 mv^2

Question 9

RMS Velocity

Answer 9

Depends of Mass and Temperature

Question 10

RMS Formula

Answer 10

urms = sqrt of 3RT / M

Question 11

Gas Constant (R)

Answer 11

8.314 J / Mol x K

Question 12

Maxwell Boltzmann Distribution of gases

Answer 12

T is related to Avg. KE

Question 13

Mean Free Path

Answer 13

Path of a particle before collision with another

Question 14

Diffusion

Answer 14

Heavier = Diffuse Slowly
Lighter = Diffuse quickly

Question 15

Effusion

Answer 15

Rate proporcional a 1 / sqrt of M

Question 16

Grahams Law Formula

Answer 16

Rate A / Rate B = sqrt of M of B / M of A

Question 17

Ideal Behavior (Real Gases)

Answer 17

-High Temperature
-Low Pressure
-Large Volume
-Small Gas Particle Size
-Least Intermoleculare Attraction Forces

Question 18

Interaction Between Water and Compounds

Answer 18

Ion-Dipole

Question 19

Is Ion-Dipole stronger than Hydrogen Bonding?

Answer 19

Yes

Question 20

Molarity Formula

Answer 20

Molarity = Moles of CHemicall / Liter

Question 21

Particle Models Represent

Answer 21

-Interaction Between Components

-Concentration of Components